l ( How many carbon atoms are there in 1.0 mole of sucrose? (Avogadro's number 6.022 x 1023) (c) (i) Define "lattice energy" ofreaction? (ii) Draw the Bond-Haber cycle for NaCl and use the data below to calculáte its lattice energy. AH (KJ) Reaction 109 + Na(g) + 2CI (g) Na (s)- 243 Cl2 (g) Na (g) 496 Na* (g) + e -349 CI (g) + e - CI (g) -411 Na(s) + 1/2C12 (g)

l ( How many carbon atoms are there in 1.0 mole of sucrose? (Avogadro's number 6.022 x 1023) (c) (i) Define "lattice energy" ofreaction? (ii) Draw the Bond-Haber cycle for NaCl and use the data below to calculáte its lattice energy. AH (KJ) Reaction 109 + Na(g) + 2CI (g) Na (s)- 243 Cl2 (g) Na (g) 496 Na* (g) + e -349 CI (g) + e - CI (g) -411 Na(s) + 1/2C12 (g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following reactions: AH = -393.5 kJ (graphite) + 2 AH = -285.8 kJ 2(g) CH,OH + 3/2 0, +2H,0 AH = -726.4 k (1) Choose... Choose... -48.25 Calculate the enthalpy change for the following reaction: 188.7 + 2 H29) CH,OH -37.6 C (graphite) + V½ 0, 10.7 -238.7 39.0 268 11.85 Given the following information: N, bond energy = 941 kJ/mol, F, bond energy = 154 kJ/mol 2 N + 3/2 F AH = -103 kJ/mol 2(g) Choose... Calculate the N-F bond energy (kJ/mol) A ballon originally had a volume of 8.68 L at 258 K and a pressure of 575 mmHg. To what temperature (in K) must the balloon be cooled to reduce its volume to 5.00 L at a pressure of 730 mmHg? Choose... V
Determine the change in enthalpy (kJ/mol) for the following reaction. Use significant figures CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) H=?
(D 263 kJ/mol P. 22. Using the following thermochemical equations: C(s) + O,(g) → CO,(g) ΔΗΟ. rxn 1 =-394 kJ/mol,Txn C(s) + CO,(g) → 2 CO(g) AH°. Ixn 2 =+173 kJ/mol,xa Determine the enthalpy of the reaction represented below: 2 C(s) + 0,(g) → 2 CO(g) ΔΗ Txn 3 = ? 1> (A) ΔΗ. :-567 kJ/molxn rxn (В) ДН =-221 kJ/mol,xn (С) ДН =+221 kJ/molpxn (D) AH°. +567 kJ/molpxn %3D Ixn qt ian od geind hw qua boalunai na cop d ofiosa orb d A 100--32 HO0-02 X convinn or rmrainn an nart of this nanA iR llanal.
changé if 1.25 g of NO is completely converted into NO,? #36. Acetic acid, CH3CO2H, is made industrially by the reaction by the reaction of methanol and carbon monoxide. CH3OH(I) + CO2(g) CH;CO2H (1) H= -134,6 KJ/mol-rxn What is the enthalpy change for producing 1.00L of acetic acid ( d= 1.044g/mL) by this reaction? Op
The heat gained by the solution in reaction two is 5.3 kJ. how many moles of NaOH were consumed ? what was the enthalpy of reaction ? (In kJ/mole)
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note…
a) Using standard enthalpies of formation (in Appendix G in your text), calculate the standard enthalpy change (AH°) for the following reaction shown below. (Show all work.) b) Based on your calculation, is the reaction exothermic or endothermic? 2 H2S(g) + SO2(g) --> 3/8 S8(s) + 2 H20(g)
Fluorine (F2), the most electronegative element reacts with water in a different way compared to other halogens do. With excess water, fluorine reacts with water to produce hydrofluoric acid and oxygen gas in the following reaction: 2F2(g) + 2H2O() →4HF (1) + O2(g) Calculate AHrxn for the process above from the following information: AH= +571.6 kJ (a) AH= +542.0 kJ (b) 2H₂O(1)→ 2H2(g) + O2(g) 2HF (g) → H2(g) + F2(g) Which equation(s) will you flip? O a. Only equation (b) O b. Only equation (a) O c. Both equations will be flipped. O d. No equations will be flipped.
5(a)
(3)
Please don't provide handwritten solution ....
2 C,H,0(g) + 50,(8) 4 CO2(g) + 4 H,0(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. exothermic Is this reaction exothermic, endothermic, or neither? endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. kJ kJ Calculate the reaction enthalpy AH, per mole of C,H¸0. rxn mol